What is the pH of a solution prepared by mixing 60.0 mL of 0.20M potassium carbonate...

What is the pH of a solution prepared by mixing 60.0 mL of 0.20M potassium carbonate (K2CO3) with 140.0 mL of 0.1M potassium bicarbonate (KHCO3)? a. 6.43 b. 6.30 c. 6.67 d. 10.32 e. 10.18

Solutions

Expert Solution

Answer – Given, [K₂CO₃] = [CO₃^2-] = 0.20 M

[KHCO₃] = [HCO₃^-] = 0.10 M

Moles of CO₃^2- = 0.20 M * 0.060 L

= 0.012 moles

Moles of HCO₃^- = 0.10 M * 0.140 L

= 0.014 moles

New concentration

Total volume = 140+60 = 200 mL

[CO₃^2-] = 0.012 moles / 0.200 L = 0.06 M

[HCO₃^-] = 0.0140 / 0.200 L = 0.07 M

We know the pKa2 for H₂CO₃ = 10.25

We know the Henderson Hasselbalch equation –

pH = pKa2 + log [CO₃^2-] / [HCO₃^-]

= 10.25 + log 0.06 / 0.07

= 10.18

So the pH of a solution prepared by mixing 60.0 mL of 0.20M potassium carbonate (K2CO3) with 140.0 mL of 0.1M potassium bicarbonate (KHCO3) is e ) 10.18

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A solution prepared by mixing 60.0 mL of 0.220 M AgNO3 and 60.0 mL of 0.220...

A solution prepared by mixing 60.0 mL of 0.220 M AgNO3 and 60.0 mL of 0.220 M TlNO3 was titrated with 0.440 M NaBr in a cell containing a silver indicator electrode and a reference electrode of constant potential 0.175 V. The reference electrode is attached to the positive terminal of the potentiometer, and the silver electrode is attached to the negative terminal. The solubility constant of TlBr is Ksp = 3.6 × 10–6 and the solubility constant of AgBr...

a) What is the pH of a buffer solution prepared by mixing 120 mL of a...

a) What is the pH of a buffer solution prepared by mixing 120 mL of a 0.435 M CH3CO2H with 50 mL of a .286 M CH3CO2Na solution? CH3CO2H Ka = 1.75 x 10-5 b) What is the resulting pH if we add 10.2 mL of a .513 M HCl solution to this buffer? Does the pH make sense? Why/why not? c) What is the resulting pH if we add 3.56 mL of a 0.420 M NaOH solution to the...

What is the pH of a solution prepared by mixing 25 ml of 0.5 HCN with...

What is the pH of a solution prepared by mixing 25 ml of 0.5 HCN with 75 ml of 0.20 NaCN. Ka = 6.2*10^-10 for HCN. Hint: remember to dilutions first.

Refer to the equilibrium constants. Calculate the pH of a solution prepared by adding 60.0 mL...

Refer to the equilibrium constants. Calculate the pH of a solution prepared by adding 60.0 mL of 0.100 M NaOH to 100. mL of 0.100 M CH3COOH solution (CH3COOH Ka = 1.8*10^-5) . Answer is B, please show work. A)4.56 B)4.92 C)5.00 D)5.08 E)5.16

1. Determine the pH of the buffer solution that is prepared by mixing 259 mL of...

1. Determine the pH of the buffer solution that is prepared by mixing 259 mL of 0.0983 M BIS−TRIS propane−H (C11H27N2O6+ ) to 855 mL of 0.0729 M BIS-TRIS_propane (C11H26N2O6) ). Assume the 5% approximation is valid. Report your answer to 2 decimal places. The pKa of BIS−TRIS propane−H is 9.10. Submit Answer Tries 0/3 2. Determine the pH of the BIS−TRIS propane−H/BIS−TRIS propane buffer solution after the addition of 25.2 mL of 0.643 M solution of rubidium hydroxide to...

Question